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Papessa [141]
3 years ago
13

Determine the mass of CaCO3 required to produce 40.0 mL CO2 at STP. Hint use molar volume of an ideal gas (22.4 L)

Chemistry
1 answer:
cupoosta [38]3 years ago
3 0

Answer:

m_{CaCO_3}=0.179gCaCO_3

Explanation:

Hello,

In this case, since the undergoing chemical reaction is:

CaCO_3(s)\rightarrow CaO(s)+CO_2(g)

The corresponding moles of carbon dioxide occupying 40.0 mL (0.0400 L) are computed by using the ideal gas equation at 273.15 K and 1.00 atm (STP) as follows:

PV=nRT\\\\n=\frac{PV}{RT}=\frac{1.00 atm*0.0400L}{0.082\frac{atm*L}{mol*K}*273.15 K})=1.79x10^{-3} mol CO_2

Then, since the mole ratio between carbon dioxide and calcium carbonate is 1:1 and the molar mass of the reactant is 100 g/mol, the mass that yields such volume turns out:

m_{CaCO_3}=1.79x10^{-3}molCO_2*\frac{1molCaCO_3}{1molCO_2} *\frac{100g CaCO_3}{1molCaCO_3}\\ \\m_{CaCO_3}=0.179gCaCO_3

Regards.

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First Set of Answers:

Heat Released Reaction 1: 3700

Heat Released Reaction 2: 3200

Second Set of Answers:

Moles Reactant 1: .00823

Moles Reactant 2: .0397

Third Set of Answers:

Enthalpy 1: -450

Enthalpy 2: -81

FOR EDG!!!!!!!!!!!!

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8 0
3 years ago
Which of the following lists characteristics of a lake and NOT a reservoir A. Artificial dam, fresh water B. natural dam, filled
tester [92]
<span>Which of the following lists characteristics of a lake and NOT a reservoir A. Artificial dam, fresh water B. natural dam, filled by runoff C. earth dam, salt water D. filled by erosion, cement dam
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4 0
3 years ago
Read 2 more answers
You have 17 liters of gas at STP. If the temperature rises to 94C and while the volume decreases to 12 liters, what will the ne
fenix001 [56]

Answer:

P_2=1.90atm

Explanation:

Hello!

In this case, according to the ideal gas equation ratio for two states:

\frac{P_1V_1}{P_2V_2} =\frac{n_1RT_1}{n_2RT_2}

Whereas both n and R are cancelled out as they don't change, we obtain:

\frac{P_1V_1}{P_2V_2} =\frac{T_1}{T_2}

Thus, by solving for the final pressure, we obtain:

\frac{P_2V_2}{P_1V_1} =\frac{T_2}{T_1}\\\\P_2=\frac{T_2P_1V_1}{V_2T_1}

Now, since initial conditions are 1.00 atm, 273.15 K and 17 L and final temperature and volume are 94 + 273 = 367 K and 12 L respectively, the resulting pressure turns out to be:

P_2=\frac{367K*1.00atm*17L}{12L*273.15K}\\\\P_2=1.90atm

Best regards!

7 0
3 years ago
A 24.00 mL sample of a solution of Pb(ClO3)2 was diluted with water to 52.00 mL. A 17.00 mL sample of the dilute solution was fo
klio [65]

Answer:

0.238 M

Explanation:

A 17.00 mL sample of the dilute solution was found to contain 0.220 M ClO₃⁻(aq). The concentration is an intensive property, so the concentration in the 52.00 mL is also 0.220 M ClO₃⁻(aq). We can find the initial concentration of ClO₃⁻ using the dilution rule.

C₁.V₁ = C₂.V₂

C₁ × 24.00 mL = 0.220 M × 52.00 mL

C₁ = 0.477 M

The concentration of Pb(ClO₃)₂ is:

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4 0
3 years ago
A sample of C3H8 has 6.72 x 10^24 H atoms. <br> What is the total mass of the sample?
gregori [183]
The answer is 492.8 g


1. Calculate a number of moles of a sample.
2. Calculate a molar mass of C3H8.
3. Calculate a mass of the sample. 

1. Avogadro's number is the number of units (atoms, molecules) in 1 mole of substance: 6.023 × 10²³ units per 1 mole    

6.023 × 10²³ atoms : 1 mol =6.72 × 10²⁴ atoms : n

n = 6.72 × 10²⁴ atoms * 1 mol : 6.023 × 10²³ atoms = 1.12 × 10 mol = 11.2 mol


2. Molar mass (Mr) of C3H8 is sum of atomic masses (Ar) of its elements:

Ar(C) = 12 g/mol

Ar(H) = 1 g/mol

Mr(C3H8) = 3 * Ar(C) + 8 * Ar(H) = 3 * 12 + 8 * 1 = 36 + 8 = 44 g/mol



3. Mass (m) of a sample is number of moles (n) multiplied by molar mass (Mr) of C3H8:

m = n * Mr = 11.2 mol * 44 g/mol = 492.8 g

6 0
2 years ago
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