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fiasKO [112]
3 years ago
9

Consider the reaction: 2 HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2 H2O(l); H = –118 kJ. Calculate the change in temperature when 50.

0 mL of 0.20 M HCl(aq) and 50.0 mL of 0.10 M Ba(OH)2(aq) are mixed together. The density ofthe solution is 1.00 g/mL and Solution= 4.184 J/g-°C
Chemistry
1 answer:
Alborosie3 years ago
6 0

Answer:

ΔT = 1,41°C

Explanation:

For the reaction:

2HCl(aq) + Ba(OH)₂(aq) → BaCl₂(aq) + 2 H₂O(l); ΔH = –118 kJ.

If moles of reaction are:

HCl:

0,0500L×0,20M = 0,01moles

Ba(OH)₂:

0,0500L×0,10M = 0,005moles

The heat produced is:

0,005mol×-118 kJ/mol = -0,59 kJ = -590 J

The temperature increasing is:

Q = -C×m×ΔT

Where Q is heat (-590 J), m is mass of solution (100mL = 100g -density of 1,00g/mL) and ΔT is change in temperature.

Replacing:

-590J = -4,184J/g°C×100g×ΔT

<em>ΔT = 1,41°C</em>

<em></em>

I hope it helps!

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A student collects 350 mL of a vapor at a temperature of 67°C. The atmospheric pressure at the time of collection is 0.900 atm.
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Answer:

Explanation:

This problem is very similar to the other that you put before, so, we'll use the same principle here.

The ideal gas equation: PV = nRT

Where:

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to get the molar mass of the gas, we need to know the moles, and with the mass, we can know the molar mass. However we can put the ideal gas expression with the molar mass in this way:

we know that n is mole so:

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Now, the closest answer of your options would be 72 g/mol. This could be easily explained because we do not use all the significant figures of all numbers, including the gas constant of R. However, all the work, calculations and procedure is correct and fine, and we only have a minimum range of 2 units.

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