Question

In: Chemistry

A 1.000 g-sample of a compound undergoes combustion in a bomb calorimeter. The temperature of the...

A 1.000 g-sample of a compound undergoes combustion in a bomb calorimeter. The temperature of the calorimeter rises from 12.0 ^oC to 70.8 ^oC. If the heat capacity of the calorimeter is 810.1 J/^oC, determine the change in internal energy for the combustion reaction,

ΔΔ

ΔΔE_rxn, in kJ/mol. The molar mass of the compound is 142.32 g/mol.

What is the energy change associated with 3.5 mol of D being formed?

2 B + C

⟶⟶

⟶⟶ D + E

ΔΔ

ΔΔH_rxn = -24.0 kJ

Select the fully correct statement.

Group of answer choices

If the products have a lower internal energy than the reactants, the change in internal energy for the system is negative and energy flows into the system from the surroundings.

If the products have a lower internal energy than the reactants, the change in internal energy for the system is positive and energy flows into the system from the surroundings.

If the reactants have a lower internal energy than the products, the change in internal energy for the system is negative and energy flows into the surrounding from the system.

If the reactants have a lower internal energy than the products, the change in internal energy for the system is positive and energy flows into the system from the surroundings.

The air in a He balloon (the system) warms over a fire and absorbs 115 J of heat. As it expands, it does 77 J of
work. What is the change in internal energy for the system?

Expert Solution

queen_honey_blossom answered 2 years ago

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