In the reaction AgNO3(aq) + HCl(aq) AgCl(s) + HNO3(aq) + heat, when 0.70 mole of AgNO3 and 0.70 mole of HCl react, the temperature of 50 g of water increases from 15°C to 30°C. If the specific heat of water is 4.18 J/g•°C, how much energy was produced in the AgNO3 reaction?
A. 2100 J
B. 42 J
C. 1050 J
D. 3100 J
The answer I got was 3135.
I obtained 3538; I suspect D is the correct answer since the 0.70 mols restricts the answer to 2 significant figure and 3100 is that. Technically the 50 number of grams H2O has only 1 s.f. but I guess they ignored that.
To solve this problem, we need to calculate the energy produced in the AgNO3 reaction using the equation q = mcΔT, where q is the energy produced, m is the mass of water, c is the specific heat of water, and ΔT is the change in temperature.
First, let's calculate the mass of water. We are given that the temperature of 50 g of water increased from 15°C to 30°C, so the change in temperature (ΔT) is 30°C - 15°C = 15°C.
Next, let's substitute the known values into the equation. We know that m = 50 g and c = 4.18 J/g•°C.
q = (50 g) * (4.18 J/g•°C) * (15°C)
q = 3135 J
The energy produced in the AgNO3 reaction is 3135 J.
However, the answer choices provided are slightly different, so let's examine the options:
A. 2100 J: This is not the same as our calculated value of 3135 J.
B. 42 J: This is not the same as our calculated value of 3135 J.
C. 1050 J: This is not the same as our calculated value of 3135 J.
D. 3100 J: This is not the same as our calculated value of 3135 J.
Based on the information provided, it appears that there may be an error in the answer choices. Our calculated value of 3135 J does not match any of the given options.
To determine the amount of energy produced in the AgNO3 reaction, we need to calculate the heat absorbed by water as it undergoes a temperature change. This can be done using the equation:
q = mcΔT
Where:
q = heat absorbed or released by the water (in Joules)
m = mass of water (in grams)
c = specific heat of water (in J/g•°C)
ΔT = change in temperature (in °C)
Given:
m = 50 g (mass of water)
c = 4.18 J/g•°C (specific heat of water)
ΔT = 30°C - 15°C = 15°C (change in temperature)
Plugging in the values, we can calculate q:
q = (50 g)(4.18 J/g•°C)(15°C)
q = 3135 J
Therefore, the energy produced in the AgNO3 reaction is 3135 Joules. However, this does not correspond to any of the options provided.
It's worth noting that the given reaction does not specify the stoichiometry between AgNO3 and HCl, so we cannot determine the number of moles that reacted. Without this information, it is not possible to calculate the energy produced accurately.