Answer:
50% ISOPROPANOL / H2O - 1
25% ISOPROPANOL / H2O - 2
Pure water - 4
ISOPROPANOL / H2O - 3
Explanation:
More Isopropanol concentration is least polar. When the isopropanol is mixed with water its polarity increases. Pure water is most polar. The polarity of a substance is dependent on its ability to bent and mold in the shape as required.
Which of the following material is the weakest thermal conducters
4) The initial rate of the reaction between substances P and Q was measured in a series of
experiments and the following rate equation was deduced.
rate = k[P]?[Q]
Complete the table of data below for the reaction between P and Q
*Help asap please*
Answer:
The initial rate of the reaction between substances P and Q was measured in a series of
experiments and the following rate equation was deduced.
[tex]rate = k[P]^{2} [Q][/tex]
Complete the table of data below for the reaction between P and Q
Explanation:
Given rate of the reaction is:
[tex]rate= k[P]^{2} [Q]\\=>[Q]=\frac{rate}{k.[P]^{2} } \\and \\\\\\\ [P]=\sqrt{\frac{rate}{k.[Q]} }[/tex]
Substitute the given values in this formulae to get the [P], [Q] and rate values.
From the first row,
the value of k can be calulated:
[tex]k=\frac{rate}{[P]^{2}[Q] } \\ =\frac{4.8*10^-3}{(0.2)^{2} 2. (0.30)} \\ =0.4[/tex]
Second row:
2. Rate value:
[tex]rate =0.4* (0.10)^{2} * (0.10)\\\\ =4.0*10^-3mol.dm^-3.s^-1[/tex]
3.Third row:
[tex][Q]=\frac{rate}{k.[P]^{2} } \\ =9.6*10^-3 / (0.4 *(0.40)^{2} \\ =0.15mol.dm^{-3}[/tex]
4. Fourth row:
[tex][P]=\sqrt{\frac{rate}{k.[Q]} }\\=>[P]=\sqrt{\frac{19.2*10^-3}{0.60*0.4} } \\=>[P]=0.283mol.dm^{-3}[/tex]
What is the balanced form of the chemical equation shown below?
Zn(NO3)2(aq) + Na S(aq) → ZnS(s) + NaNO3(aq)
how many atoms of carbon are in 6CO2 + 6H2O --> C6H12O6 + 6O2
Answer:
6 atoms of carbon are in the reactant side
Explanation:
Are on the reactant side in:
6CO2 + 6H2O → C6H12O6 + 6O2
In the reaction, there are 6 molecules of CO2 that are reacting with 6 molecules of H2O. As you can see, CO2 has only 1 atom of carbon per molecule whereas H2O hasn't.
That means the atoms of carbon are:
6 molecules CO2 * (1atom C / 1molecule CO2) =
6 atoms of carbon are in the reactant sidewhich substances would have exhibit a giant covalent structure explain
Answer:
Silicon
Explanation:
Silicon is in group IV with strong Si-Si ( Silicon to Silicon ) bonds. Since it is a molecule, these bonds exert a strong molecular force hence adopting a giant covalent structure.
The student is now told that the four solids, in no particular order, are barium chloride (BaCl2), sugar (C6H12O6), butanoic acid (C3H7COOH), and sodium bromide (NaBr). Assuming that conductivity is correlated to the number of ions in solution, rank the four substances based on how well a 0.20 M solution in water will conduct electricity. Rank from most conductive to least conductive.
Answer:
The student is now told that the four solids, in no particular order, are barium chloride (BaCl2), sugar (C6H12O6), butanoic acid (C3H7COOH), and sodium bromide (NaBr). Assuming that conductivity is correlated to the number of ions in solution, rank the four substances based on how well a 0.20 M solution in water will conduct electricity. Rank from most conductive to least conductive.
Explanation:
The given substances are:
barium chloride(BaCl2),
glucose(C6H12O6),
butanoic acid (C3H7COOH) which is a weak acid,
sodium bromide (NaBr).
The conductivity of a solution is proportional to the number of ions present in a particular solution.
1mol. of BaCl2 in water produces a total three mol. of ions.
[tex]BaCl_2 (aq) -> Ba^2^+(aq) + 2Cl^-(aq)[/tex]
Gluocse is a covalent compound and it does not dissociate into ions in water.
So, it does not conduct electricity.
Butanoic acid is a weak acid. But due to the release of H+ ions it can conduct a very less amount of electricity.
NaBr is an ionic compound and in 1mol. of NaBr in water gives two mol. of ions.
NaBr (aq) -> Na+ (aq) + Br- (aq)
Hence, the order of conductivity among the given substances in aqueous solution is:
BaCl2 > NaBr > butanoic acid > glucose
Calculate the mass percent composition of O in each compound.
a. calcium nitrate
b. Iron(II) sulfate
c. Carbon dioxide
Answer:
A. Mass percent composition of oxygen = 58.5%
B. Mass percentage composition of oxygen = 42.1%
C. Mass percentage composition of oxygen = 72.7 %
Explanation:
Percentage mass composition of an element in a compound is given by the formula below:
Percentage mass composition = mass of element/ molar mass of compound × 100%
Percentage mass of oxygen in the given compounds are then calculated.
a. Calcium nitrate, Ca(NO₃)₂: molar mass of compound is obtained first.
Molar mass of Ca(NO₃)₂ = 40 + 14 × 2 + 16 × 2 × 3 = 164 g
Mass of oxygen = 16 × 6 = 96 g
Mass percent composition of oxygen = 96/164 × 100% = 58.5%
b. Iron (ii) sulfate, FeSO₄: molar mass of compound is obtained first.
Molar mass of FeSO₄ = 56 + 32 + 16 × 4 = 152 g
Mass of oxygen = 16 × 4 = 64 g
Mass percentage composition of oxygen = 64/152 × 100% = 42.1%
c. Carbon dioxide, CO₂: molar mass of compound is obtained first.
Molar mass of CO₂ = 12 + 16 × 2 = 44 g
Mass of oxygen = 16 × 2 = 32 g
Mass percentage composition of oxygen = 32/44 × 100% = 72.7 %
A worker gets paid 11.33 $/hour. The worker works on average 39.7 hours/week for 48 weeks per year. How much does the worker make in 1.7 years?
Answer:
36704 $
Explanation:
First we calculate how much the worker gets paid in one week:
11.33 $/hour * 39.7 hour/week = 449.80 $/weekThen we calculate how many weeks does the worker work in 1.7 years:
48 week/year * 1.7 years = 81.6 weeksFinally we calculate how much does the worker make in 1.7 years:
449.80 $/week * 81.6 weeks = 36704 $When 1.00 g of coal is burned in a bomb calorimeter, the temperature increases by 1.48°C. If the heat capacity of the calorimeter is 21.6 kJ/°C, determine the heat (in GJ) produced by combustion of a ton of coal.
Answer:
32.0 kJ
General Formulas and Concepts:
Thermochemistry
Specific Heat Formula: q = mcΔT
q is heat (in J) m is mass (in g) c is specific heat (in J/g °C) ΔT is change in temperature (in °C)Explanation:
Step 1: Define
Identify variables
[Given] m = 1.00 g
[Given] ΔT = 1.48 °C
[Given] c = 21.6 kJ/g °C
[Solve] q
Step 2: Find Heat
Substitute in variables [Specific Heat Formula]: q = (1.00 g)(21.6 kJ/g °C)(1.48 °C)Multiply [Cancel out units]: q = (21.6 kJ/°C)(1.48 °C)Multiply [Cancel out units]: q = 31.968 kJStep 3: Check
Follow sig fig rules and round. We are given 3 sig figs.
31.968 kJ ≈ 32.0 kJ
Consider the reaction between solid C and O2 gas which makes CO2;
C+02 -> CO2
If we have a 14 L container of O2 gas at a pressure of 3.0 atm and a temperature of 298 K and we add 36 g of solid C to the
container, then how many grams of CO2 will be produced by this reaction?
Answer:
[tex]m_{CO_2}=75.6gCO_2[/tex]
Explanation:
Hello there!
In this case, according to the given information, it turns out mandatory for us to calculate the reacting moles of both C and O2 because we are given grams and pressure, temperature and volume, respectively:
[tex]n_C=36gC*\frac{1molC}{12gC}=3.0molC \\\\n_{O_2}=\frac{3.0atm*14L}{0.08206\frac{atm*L}{mol*K}*298K}=1.72molO_2[/tex]
Thus, since C and O2 react in a 1:1 mole ratio, we infer C is in excess, and the grams of CO2 can be calculated with the moles of O2:
[tex]m_{CO_2}=1.72molO_2*\frac{1molCO_2}{1molO_2}*\frac{44.01gCO_2}{1molCO_2} \\\\ m_{CO_2}=75.6gCO_2[/tex]
Best regards!
A buffer solution is prepared by adding 13.74 g of sodium acetate (NaC2H3O2) and 15.36 g of acetic acid to enough water to make 500 mL (three significant figures) of solution. Calculate the pH of this buffer.
Answer:
A buffer solution is prepared by adding 13.74 g of sodium acetate (NaC2H3O2) and 15.36 g of acetic acid to enough water to make 500 mL of solution.
Calculate the pH of this buffer.
Explanation:
The pH of a buffer solution can be calculated by using the Henderson-Hesselbalch equation:
[tex]pH=pKa+log\frac{[salt]}{[acid]}[/tex]
The pH of the given buffer solution can be calculated as shown below:
A 10.0 g gold ring with a specific heat 0.129 at 24.00°C is placed in a calorimeter with 118 g of water at 1.00°C.
What will be the final temperature of the system?
Answer:
1.06 °C
Explanation:
From the question given above, the following data were obtained:
Mass of gold (M₉) = 10 g
Specific heat capacity of gold (C₉) = 0.129 J/gºC
Initial temperature of gold (T₉) = 24 °C
Mass of water (Mᵥᵥ) = 118 g
Specific heat capacity of water (Cᵥᵥ) = 4.184 J/gºC
Initial temperature of water (Tᵥᵥ) = 1 °C
Equilibrium temperature (Tₑ) =?
The equilibrium temperature of the system can be obtained as follow:
Heat loss by the gold = heat gained by the water
M₉C₉(T₉ – Tₑ) = MᵥᵥCᵥᵥ(Tₑ – Cᵥᵥ)
10 × 0.129 (24 – Tₑ) = 118 × 4.184 (Tₑ – 1)
1.29(24 – Tₑ) = 493.712 (Tₑ – 1)
Clear bracket
30.96 – 1.29Tₑ = 493.712Tₑ – 493.712
Collect like terms
30.96 + 493.712 = 493.712Tₑ + 1.29Tₑ
524.672 = 495.002Tₑ
Divide both side by 495.002
Tₑ = 524.672 / 495.002
Tₑ = 1.06 °C
Therefore, the temperature of the system is 1.06 °C
The amount of heat of the system is measured by a device called a calorimeter. The final temperature of the system will be 1.06 degrees celsius.
What is equilibrium temperature?The equilibrium temperature is the temperature that follows the law of thermodynamics and is said to be the system that has alike temperatures.
Given,
Mass of Ag [tex]\rm (M_{g})[/tex] = 10g
Specific heat capacity of Ag [tex](\rm C_{g})[/tex] = [tex]\rm 0.129 J/g^{\circ}C[/tex]
The initial temperature of Ag [tex](\rm T_{g})[/tex] = [tex]24 ^{\circ}\;\rm C[/tex]
Mass of water [tex](\rm M_{w})[/tex] = 118 g
Specific heat capacity of water [tex](\rm C_{w})[/tex] = [tex]4.184 \rm \;J/g^{\circ}\;\rm C[/tex]
The initial temperature of water [tex](\rm T_{w})[/tex] = [tex]1 ^{\circ}\;\rm C[/tex]
Equilibrium temperature = [tex](\rm T_{e})[/tex]
The equilibrium temperature can be shown as, heat loss by the gold = heat gained by the water:
[tex]\rm \rm M_{g}C_{g}(T_{g} - T_{e}) = M_{w}C_{w}(T_{e}-C_{w})[/tex]
Substituting values in the equation:
[tex]\begin{aligned} 10 \times 0.129 (24 - \rm T_{e}) &= 118 \times 4.184 (\rm T_{e} - 1)\\\\\rm 1.29(24 - T_{e}) &= 493.712 (\rm T_{e} - 1)\\\\524.672 &= 495.002 \;\rm T_{e}\end{aligned}[/tex]
Now divide both the sides by 495.002:
[tex]\begin{aligned} \rm T_{e} &= \dfrac{524.672 }{495.002}\\\\\rm T_{e} &= 1.06 \;^{\circ}\rm C\end{aligned}[/tex]
Therefore, the final temperature of the system is 1.06 degrees celsius.
Learn more about equilibrium temperature here:
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Examine the differences between the expanded structure, the condensed structure, and bond-line representation.
Answer:
One structure shows all the bonds whereas the other shows some of the bonds.
Explanation:
Expanded structure shows all of the bonds connecting all of the atoms in the compound while on the hand, condensed structural shows all atoms, but exclude some or all of the vertical and horizontal bonds. condensed structure makes it easier to write the formula in a line as compared to expanded structure. A bond-line representation is a kind of representation of molecular structure of compounds on a line. In this representation, covalent bonds are represented with one line for each level of bond order.
A small coffee cup calorimeter contains 28.0 g of H2O at 19.73 oC. A 2.05 g sample of a metal alloy is heated to 98.88 oC and then placed in the water. The contents of the calorimeter come to a temperature of 21.23 oC. What is the specific heat of lead
Answer:
1.104 J/g°C
Explanation:
Using Q = m × c × ∆T
Where;
m = mass of substance (g)
c = specific hear capacity (J/g°C)
∆T = change in temperature (°C)
For a colorimeter,
Q(water) = - Q(metal)
m. c. ∆T (water) = - m. c. ∆T (metal)
According to the information provided;
For water:
m = 28.0g
c = 4.184 J/g°C
∆T = (21.23 - 19.73°C)
For the metal:
m = 2.05g
c = ?
∆T = (21.23 - 98.88°C)
m. c. ∆T (water) = - m. c. ∆T (metal)
[28 × 4.184 × (21.23 - 19.73°C)] = -[2.05 × c × (21.23 - 98.88°C)]
[117.152 × 1.5] = -[2.05 × c × (-77.65)]
175.728 = -[-159.1825c]
175.728 = 159.1825c
c = 175.728 ÷ 159.1825
c = 1.104
c = 1.104 J/g°C
please help me asap!!
Answer:
Al2o3 is 101
(nh4)2O IS 52
S8 is 256.56
Ba(oh)2 is 171.35
Cacl2 is 110.98
H2O is 18.01
Explanation:
The molecules you use in a chemical reaction are called the:
a) If we have a 4.5 L container of CH 10 gas at a temperature of 178 K and a pressure of 0.50 atm, then how many moles of CaHio do
we have?
b) How many grams of C4H1o do we have?
Answer:
a) 0.15 mol.
b) 8.95 g.
Explanation:
Hello there!
In this case, according to the given information, it is possible for us to infer this problem is solved by using the ideal gas equation:
[tex]PV=nRT[/tex]
And proceed as follows:
a) Here, we solve for the moles, n, as follows:
[tex]n=\frac{PV}{RT} \\\\n=\frac{0.50atm*4.5L}{0.08206\frac{atm*L}{mol*K}*178K} \\\\n=0.15mol[/tex]
b) for the calculation of the mass, we recall the molar mass of butane, 58.12 g/mol, to obtain:
[tex]0.15mol*\frac{58.12g}{1mol} =8.95g[/tex]
Regards!
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An alkyl groyp has a formula of CxH6, determine the value of x
Answer:
i didnt understand
Explanation:
Answer:
x = 2 (C₂H₆)
Explanation:
The general formula for alkanes is CₓH₂ₓ₊₂
2x + 2 = 6
Simply solve for n:
2x = 4
x = 2
Determine how much sulfuric acid (in metric tons) is produced by the combustion of 1.2 metric ton of this coal. (A metric ton is 1000 kg.)
A small container is filled with liquid water. What can happen if the container of water is an open system that couldn't happen if it were a closed or isolated system?
Evaporation can decrease the amount of water. Dust from the surroundings can enter the water. The water can freeze if the surrounding temperature decreases sufficiently.
We have a 3.7 L container filled with 82 g of CO gas. This container is maintained at a temperature of 298 K
a) How many moles of CO gas are in this container?
b) What is the pressure inside the container?
Answer:
a) 2.9 mol
b) 19 atm
Explanation:
Step 1: Given data
Volume of the container (V): 3.7 LMass of CO gas (m): 82 gTemperature (T): 298 KStep 2: Calculate the number of moles (n) corresponding to 82 g of CO
The molar mass of CO is 28.01 g/mol.
82 g × 1 mol/28.01 g = 2.9 mol
Step 3: Calculate the pressure (P) inside the container
We will use the ideal gas equation.
P × V = n × R × T
P = n × R × T / V
P = 2.9 mol × (0.0821 atm.L/mol.K) × 298 K / 3.7 L = 19 atm
All forms of energy can exist as either ________ or ________ energy.
Answer:
potentiol or kenetic
Explanation:
A solution of permanganate is standardized by titration with oxalic acid, . To react completely with mol of oxalic acid required 28.18 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is Determine the concentration of the permanganate solution in molarity. g
The question is incomplete, the complete question is:
A solution of permanganate is standardized by titration with oxalic acid. To react completely with 0.0018 mol of oxalic acid required 28.18 mL of permanganate solution. The unbalanced chemical equation for the reaction in acidic solution is:
[tex]\mathrm{MnO}_{4}^{-}(aq)+\mathrm{H}_{2}\mathrm{C}_{2}\mathrm{O}_{4}(aq)\stackrel{\mathrm{Acidic}}{\longrightarrow}\mathrm{Mn}^{2+}(aq)+\mathrm{CO}_{2}(\mathrm{g})[/tex]
Determine the concentration of the permanganate solution in molarity.
Answer: The molarity of permanganate solution is 0.026 M
Explanation:
The balanced chemical equation follows:
[tex]2MnO_4^-(aq)+6H^+(aq)+5H_2C_2O_4(aq)\rightarrow 2Mn^{2+}+8H_2O(l)+10CO_2(g)[/tex]
Given values:
Moles of oxalic acid = 0.0018 moles
By the stoichiometry of the reaction:
If 5 moles of oxalic acid reacts with 2 moles of permanganate solution
So, 0.0018 moles of oxalic acid will react with = [tex]\frac{2}{5}\times 0.0018mol=0.00072mol[/tex] of permanganate solution
Molarity is defined as the amount of solute expressed in the number of moles present per liter of solution. The units of molarity are mol/L. The formula used to calculate molarity:
[tex]\text{Molarity of solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (mL)}}[/tex] .....(1)
Given values:
Moles of permanganate solution = 0.00072 moles
Volume of solution = 28.18 mL
Putting values in equation 1, we get:
[tex]\text{Molarity of permanganate solution}=\frac{0.00072\times 1000}{28.18}\\\\\text{Molarity of permanganate solution}=0.026M[/tex]
Hence, the molarity of permanganate solution is 0.026 M
Which compound is insoluble in water?
Answer:
The answer is C... I am almost positive.
This diagram represents chlorine monofluoride.
The arrow shows that the bond between the chlorine atom and the fluorine atom is
. The electrons in the bond are pulled
, and the chlorine atom is
.
The fluorine atom is partially negatively charged while chlorine is partially positively charged.
What are polar molecules?Polar molecules are molecules whose molecules are partially charged due to the electronegative differences between the atoms in the molecule of the compound.
Chlorine monofluoride is a polar molecule.
Fluorine is more electronegative than the chlorine atom.
Therefore, the fluorine atom is partially negatively charged while chlorine is partially positively charged.
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how to test for the presence of water in a substance
Answer:
it is...
Explanation: Pure copper(II) sulfate is white. It is also known as anhydrous copper(II) sulfate because it has no water in it. When water is present in a sample of copper(II) sulfate it turns blue.
Answer:
put it in a beaker then tne beaker in a boiling water bath and when it temperature has reached 100°c condense that gas ... if there is no gas evaporating by 100° then there is no water
Explanation:
water evaporates at 100°c
Aluminum metal reacts with oxygen gas in a combination reaction that forms a product that coat the metal preventing it from further oxidation. Which of the following is the correct balanced equation for the reaction?
a. Al(s) + 302(g) → 2903(s).
b. 2Al(s) + O2(g) → 2A10(s).
c. AI(s) + O2(g) → AIO (s).
d. 4Al(s) + 3O2(g) →2Al2O3.
e. 3Al(s) + O2 → Al3O2.
Answer:
d. 4 Al(s) + 3 O₂(g) → 2 Al₂O₃(s)
Explanation:
Aluminum metal reacts with oxygen gas in a combination reaction that forms a product that coats the metal preventing it from further oxidation: aluminum oxide. Aluminum is a cation with charge 3+ (Al³⁻) and oxide is an anion with charge 2- (O²⁻). Thus, the neutral compound aluminum oxide has the chemical formula Al₂O₃. The unbalanced chemical equation is:
Al(s) + O₂(g) → Al₂O₃(s)
We can balance using the trial and error method. First, we will balance O atoms by multiplying Al₂O₃ by 2 and O₂ by 3.
Al(s) + 3 O₂(g) → 2 Al₂O₃(s)
Finally, we get the balanced equation by multiplying Al by 4.
4 Al(s) + 3 O₂(g) → 2 Al₂O₃(s)
Which of the following is an organic compound?
ammonia (NH3)
calcium sulfide (CaS)
octane (C8H18)
sulfur trioxide (SO3)
Organic compround is octane C8H18
Excess HCl is added to 234 g of Na2S solution as shown by the equation below:
Na2S(aq) + 2HCl(aq) →2NaCl(aq) + H2S(g)
How many liters of H2S gas are produced at standard temperature and pressure (STP)? The molar mass of Na2S is 78 g.
Answer:
67 L
Explanation:
Step 1: Write the balanced equation
Na₂S(aq) + 2 HCl(aq) → 2 NaCl(aq) + H₂S(g)
Step 2: Calculate the moles corresponding to 234 g of Na₂S
The molar mass of Na₂S is 78 g/mol.
234 g × 1 mol/78 g = 3.0 mol
Step 3: Calculate the moles of H₂S produced from 3.0 moles of Na₂S
The molar ratio of Na₂S to H₂S is 1:1. The moles of H₂S formed are 1/1 × 3.0 mol = 3.0 mol.
Step 4: Calculate the volume occupied by 3.0 moles of H₂S at STP
At STP, 1 mole of H₂S occupies 22.4 L.
3.0 L × 22.4 L/1 mol = 67 L