As per Ideal gas equation, molar mass of the gas is 5.032 g/mo
We’ll begin by calculating the number of mole of the gas. This can be obtained as follow:
Volume (V) = 1.6 L
Temperature (T) = 287 K
Pressure (P) = 0.92 atm
Gas constant (R) = 0.0821 atm.L/Kmol
Number of mole (n) =?
According to Ideal gas equation , PV = nRT
0.92 × 1.6 = n × 0.0821 × 287
1.472 = n × 23.5627
Divide by 23.5627
n = 1.176 / 23.5627
n = 0.0624 mole
Finally, we shall determine the molar mass of the gas. This can be obtained as follow:
Mass of gas = 0.314 g
Number of mole = 0.0624 mole
Mole = 
0.0624 = 
Cross multiply
0.0624 × molar mass of gas = 0.314
Divide by 0.0624
Molar mass of gas = 
Molar mass of gas = 5.032 g/mo
Therefore the Molar mass of gas is 5.032 g/mo
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Answer:
C.
Explanation:
Section 1 and section 4 are balanced.
Molecules may be similar or different on the basis of size, shape, structure and chemical composition.
<h2>Similarities and differences</h2>
Two molecules can be considered similar or different on the basis of size, shape, structure and chemical composition. The molecules in the two proposed systems are consider the same when they are similar in size, shapes, structure and chemical composition.
While on the other hand, the molecules is considered different when they have different structure and chemical composition so we can say that molecules may be similar or different on the basis of size, shape, structure and chemical composition.
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Answer:
92.9 °C
Explanation:
Step 1: Given data
- Initial volume (V₁): 450. mL
- Initial temperature (T₁): 55.0 °C
- Final volume (V₂): 502 mL
Step 2: Convert 55.0 °C to Kelvin
We will use the following expression.
K = °C + 273.15 = 55.0 + 273.15 = 328.2 K
Step 3: Calculate the final temperature of the gas
If we assume constant pressure and ideal behavior, we can calculate the final temperature of the gas using Charles' law.
T₁/V₁ = T₂/V₂
T₂ = T₁ × V₂/V₁
T₂ = 328.2 K × 502 mL/450. mL = 366 K = 92.9 °C
