Chemistry: A gas is compressed from an initial volume of 5.35 L to a final volume of 1.23 L by an external pressure of 1.00 atm. During the compression the gas releases 128 J of heat. Required: What is the change in internal energy of the gas?

1.97 ml.ExplanationMg reacts with HCl at a 1:2 ratio.Mg + 2 HCl → MgCl₂ + H₂.How many moles of atoms in 0.0240 g of Mg?The molar mass of Mg is 24.305 g/mol. In other words, the mass of one mole of Mg atoms is 24.305 gram..How many moles of HCl does it take to oxidize that of Mg?It takes 2 moles of HCl to oxidize 1 mole of Mg. As a result, it takes to oxidize of Mg. Mg is the limiting reactant, meaning that HCl is in excess. There needs to be more than HCl for Mg to be the limiting reactant.How many...

A gas is compressed from an initial volume of

Ответ:

mme58

29.01.2022

Chemistry

The change in internal energy is $\Delta U = 417331 \ J$

Explanation:

From the question we are told that

The initial volume is $V_i = 5.35 \ L$

The final volume is $V_f = 1.23 \ L$

The value of the external pressure is $P = 1.00 \ atm = 1 * 101325 = 101325 \Pa$

The energy released by the gas is $Q= -128 \ J$

The negative sign show that energy is released from the system

Generally the workdone on the gas is mathematically represented as

W = P (V_i - V_f)

substituting values

W = 101325 *(1.23 - 5.35)

$W = - 4.17*10^{5} \ J$

The change in internal energy is mathematically evaluated as

$\Delta U = Q - W$

substituting values

$\Delta U = -128 - (-4.17*10^{5})$

$\Delta U = 417331 \ J$

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Ответ:

mikayla62

13.01.2020

Chemistry

1.97 ml.

Explanation

Mg reacts with HCl at a 1:2 ratio.

Mg + 2 HCl → MgCl₂ + H₂.

How many moles of atoms in 0.0240 g of Mg?

The molar mass of Mg is 24.305 g/mol. In other words, the mass of one mole of Mg atoms is 24.305 gram.

$n = \dfrac{m}{M} = \dfrac{0.0240}{24.305} = 9.87 \times 10^{-4} \; \text{mol}$ .

How many moles of HCl does it take to oxidize that $9.87 \times 10^{-4} \; \text{mol}$ of Mg?

It takes 2 moles of HCl to oxidize 1 mole of Mg. As a result, it takes $2 \times 9.87 \times 10^{-4} = 1.97 \times 10^{-3}\; \text{mol}$ to oxidize $9.87 \times 10^{-4}\; \text{mol}$ of Mg.

Mg is the limiting reactant, meaning that HCl is in excess. There needs to be more than $1.97 \times 10^{-3}\; \text{mol}$ HCl for Mg to be the limiting reactant.

How many liters of 1.00 M HCl?

1.00 M is the same as 1.00 moles per liter.

$V = \dfrac{n}{c} = \dfrac{1.97 \times 10^{-3} \; \text{mol}}{1.00 \; \text{mol}\cdot \text{L}^{-1}} = 1.97 \times 10^{-3} \; \text{L} = 1.97 \; \text{mL}$ .

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A gas is compressed from an initial volume of 5.35 L to a final volume of 1.23 L by an external pressure of 1.00 atm. During the compression the gas releases 128 J of heat. Required:
What is the change in internal energy of the gas?

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