Can u guys check my answer??
Question: convert 24 grams of ice at -10 degrees Celsius to water at 45 degrees Celsius.
I got q= 13022 joules
Is that correct?
I don't think so. Post your work and I'll look for the error.
Q=24.0g (2.03j/gc) (10c)
Q=334j/g(24g)
Q=24g(4.184j/gc)(45c)
Added them and got q= 13022j
24.0(2.03)(10) = 487.2
4518.7
487.2 + 4518.7 = ??about 5,000+
But 334 x 24= 8016
Oh oops I see where u got the 4518.7 but don't u also have to add the middle equation??
To determine if your answer is correct, we can use the formula for specific heat capacity:
q = m * c * ΔT
where:
q is the heat energy absorbed or released (in joules),
m is the mass of the substance (in grams),
c is the specific heat capacity of the substance (in joules per gram per degree Celsius), and
ΔT is the change in temperature (in degrees Celsius).
In this case, we need to convert 24 grams of ice at -10 degrees Celsius to water at 45 degrees Celsius. Let's break down the calculations step by step:
1. Determine the heat energy required to raise the temperature of ice from -10°C to 0°C:
q1 = m * c1 * ΔT1
where:
m = 24 grams
c1 = specific heat capacity of ice (2.09 J/g°C)
ΔT1 = change in temperature = (0°C - (-10°C)) = 10°C
q1 = 24 g * 2.09 J/g°C * 10°C
q1 = 501.6 J
2. Determine the heat energy required to melt the ice at 0°C:
q2 = m * ΔHf
where:
m = 24 grams
ΔHf = heat of fusion of ice (334 J/g)
q2 = 24 g * 334 J/g
q2 = 8016 J
3. Determine the heat energy required to raise the temperature of the water from 0°C to 45°C:
q3 = m * c2 * ΔT2
where:
m = 24 grams
c2 = specific heat capacity of water (4.18 J/g°C)
ΔT2 = change in temperature = (45°C - 0°C) = 45°C
q3 = 24 g * 4.18 J/g°C * 45°C
q3 = 4527.6 J
4. Sum up the three heat energy calculations:
q_total = q1 + q2 + q3
q_total = 501.6 J + 8016 J + 4527.6 J
q_total = 13045.2 J
Therefore, the correct answer for the heat energy required to convert 24 grams of ice at -10 degrees Celsius to water at 45 degrees Celsius is approximately 13045.2 joules. Your answer of 13022 joules is very close, but not exactly correct.