If the specific heat capacity of ice is 2.10 J/(g.°C), how much heat is required to heat 530 g of ice from -45.0°C to -15.0°C?
1.) 33.400 kj
2.) 32595 J
3.) 33.4 kj
4.) 33000 J
I was out sick when we learned this please help
2.10 * 530 * (-15.0 - -45.0) = ? J
careful with sig fig
33390?
Yes.
NO ... not one of the choices ...
remember the sig fig hint
I am anomynous................................
i believe you would round it up to 33000
nevermind, 33000 is WRONG. oops
To calculate the amount of heat required to heat a substance, you can use the formula:
Q = m * c * ΔT
Where:
- Q is the heat energy in joules (J)
- m is the mass of the substance in grams (g)
- c is the specific heat capacity of the substance in J/(g.°C)
- ΔT is the change in temperature in degrees Celsius (°C)
In this case, you have:
m = 530 g (mass of ice)
c = 2.10 J/(g.°C) (specific heat capacity of ice)
ΔT = (-15.0°C) - (-45.0°C) = 30.0°C (change in temperature)
Now, let's substitute the values into the formula:
Q = 530 g * 2.10 J/(g.°C) * 30.0°C
Calculating this multiplication, we get:
Q ≈ 33,300 J
Therefore, the heat required to heat 530 g of ice from -45.0°C to -15.0°C is approximately 33,300 J.
Now, to match this result with the options provided:
1.) 33.400 kJ (33,400 J)
2.) 32,595 J
3.) 33.4 kJ (33,400 J)
4.) 33,000 J
Based on the calculation, the answer would be option 3.) 33.4 kJ.