linz6227

14.06.2021 • 

Chemistry

Calculate the following for test tubes 3 and 4, and record the results in the table: the number of moles of zinc used (Use 65.38 grams/mole as the molar mass of zinc.)

the heat absorbed by the water, in joules (Use Q = mCΔT, where 10.0 milliliters of water has a mass of 10.0 grams. Use 4.186 joules/gram degree Celsius as water’s specific heat capacity.)

the change in internal energy of the copper(II) sulfate (Assume that energy released by the copper(II) sulfate is absorbed by the water.)

the reaction enthalpy, in joules/mole

Answer these for both test tubes

Moles of zinc

Heat absorbed by water (J)

Change in internal energy (J)

Reaction enthalpy (J/mol)

Ответ:

jaida03

15.10.2022

Chemistry

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V = 22.86 L

Explanation:

Given data:

Mass of nitrogen dioxide = 45000 mg

Pressure = 1 atm

Temperature = 273 k

Volume = ?

Solution:

First of all we will convert the mass into moles.

Number of moles = mass/ molar mass

Number of moles = 45 g/ 46 g/mol

Number of moles = 1.02 mol

Now we will determine the volume at STP.

PV = nRT

V = nRT/P

V =  1.02 mol × 0.0821 atm. mol⁻¹. k⁻¹. L× 273 k / 1 atm

V = 22.86 atm. L /1 atm

V = 22.86 L

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