Item 23 Imagine you mix 50.0 mL of 2.00 M solution of CaBr 2 with 70.0 mL of 2.5

Question

Item 23

Imagine you mix 50.0 mL of 2.00 M solution of CaBr2 with 70.0 mL of 2.50 M solution of AgNO3.

Part A

Write the balanced chemical equation for the reaction.

(be sure to include the state of each component)

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Part B

Which reactant is the limiting reactant?

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Part C

What mass of AgBr will be produced?

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27.2 mL of 1.70 M NaOH is needed to titrate a 50.0 mL sample of H2SO4 to equivalence.

Part A

Write the balanced chemical equation for the reaction.

Part B

What is the concentration of the H2SO4?

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Item 21

A 17.5 L container holds 125 grams of O2 gas:

Part A

What is the pressure (in atm) if the temperature is 24°C?

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Part B

What would the pressure be if the temperature increases to 100°C?

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Item 20

Part A

What is the molarity of a 0.65 L solution that contains 135g of NaCl?

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Item 12

Part A

A 20.0 L metal container holds N2 gas with a pressure of 5.00 atm at 20.0°C. The metal container can withstand pressures of 25.5 atm before it explodes. What is the maximum temperature (in °C) the gas can reach before the metal container will fail?

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Item 9

Part A

An experiment requires 75.0 mL of a 1.25 M NaOH solution. What mass of NaOH will you need to prepare the required solution?

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Item 6

Consider the reaction: ____Al + ____Fe2O3   ____Al2O3 + ____Fe

Part A

Balance the equation.

Write the coefficients from left to right, separated by commas. For example: 1,2,3

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Part B

If you start with 53g of Al and 123g of Fe2O3, what is your limiting reactant?

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Part C

How many grams of Fe can you make?

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Part D

If you do the experiment in lab and produce 63.2 g of Fe, what is your percent yield?

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For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants.
2Na(s)+Br2(g)2NaBr(s)

Part A

4 mol Na, 4 mol Br2

Express your answer as a chemical formula.

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Part B

1.8 mol Na, 1.4 mol Br2

Express your answer as a chemical formula.

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Part C

2.5 mol Na, 1 mol Br2

Express your answer as a chemical formula.

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Part D

12.0 mol Na, 6.9 mol Br2

Express your answer as a chemical formula.

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Explanation / Answer

CaBr2 + 2AgNO3 -----> 2AgBr + Ca(NO3)2
number of moles of CaBr2 = 50 * 2/1000 = 0.1
number of moles of AgNO3 = 70 * 2.5/1000 = 0.175
1 mole of CaBr2 reacts with 2 moles of AgNO3
0.1 moles of CaBr2 reacts with 0.1*2 = 0.2 moles of AgNO3
so AgNO3 is limiting reagent.
2 moles of AgNO3 produces 2 moles of AgBr
so the AgBr moles = 0.175
mass of AgBr = 0.175 * 188 = 32.9 g

2NaOH + H2SO4 ------> Na2SO4 + 2H2O
M1V1/n1 = M2V2/n2
27.2*1.7/2 = M2*50/1
concentration of H2SO4 M2 = 0.4624

PV = m/MW*R*T
P *17.5 = 125/32 * 0.0821 *(24+273)
P = 5.442 atm
P * 17.5 = 125/32 * 0.0821 * (100+273)
P = 6.8355 atm

M = mass/MW *1/V in L
M = 135/58.5 * 1/0.65
Molarity M = 3.5503

P1/T1 = P2/T2 at constant volume
5/(20+273) = 25.5/T2
T2 = 1494.3 K beyond this temperature the container will explode.

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