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3 years ago

Values of R, the ideal gas constant, and the ideal gas equation are given below. Use these to solve the problems.

Chemistry

1 answer:

lesya [120]3 years ago

3 0

Answer:

183 K

General Formulas and Concepts:

Chemistry - Gas Laws

Combined Gas Law: PV = nRT

P is pressure
V is volume (in Liters)
n is amount of moles
R is gas constant - $0.0821 \frac{L \cdot atm}{mol \cdot K}$
T is temperature (in Kelvins)

Explanation:

Step 1: Define

10.0 L

3.00 mol H₂

4.50 atm

Step 2: Find Temperature

Substitute [CGL]: $(4.50 \ atm)(10.0 \ L) = (3.00 \ mol)(0.0821 \frac{L \cdot atm}{mol \cdot K})(x \ K)$
Isolate temperature x: $\frac{(4.50 \ atm)(10.0 \ L)}{(3.00 \ mol)(0.0821 \frac{L \cdot atm}{mol \cdot K})} = x \ K$
Rewrite: $x \ K = \frac{(4.50 \ atm)(10.0 \ L)}{(3.00 \ mol)(0.0821 \frac{L \cdot atm}{mol \cdot K})}$
Evaluate: $x = 182.704 \ K$

Step 3: Check

Round to the nearest whole number.

182.704 K ≈ 183 K

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Please I need help on these 3 questions. Thank You.

Liula [17]

V = 200 mL (volume)

c = 3 M = 3 mol/L (concentration)

First we convert mL to L:

200 mL = 0.2 L

Then we calculate the moles using the formula: n = V × c = 0.2 L × 3 mol = 0.6 mol

Finally, we just use the molar mass of CaF2 to calculate the actual mass:

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n = V × c = 0.05 L × 12 mol/L = 0.6 mol

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The steps for this question are the opposite way.

m(K2CO3) = 250 g

molar mass = 138 g/mol

n = m ÷ mm = 1.81 mol

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