If 155 J of energy is added to 18.5 g of silver, how much will the temperature rise?
Silver Specific Heat= (0.235J/g deg C)
q = mass Ag x specific heat Ag x delta T
Solve for delta T.
That's the formula I used
Delta T = 115J/18.5g(0.235J/g deg C)
= J and g cancel leaving me with deg C
=115/18.5(0.235 deg C)
=35.65 deg C
=36 deg C
my answer was wrong but I don't know correct answer
The correct answer is 35.6. You are allowed 3 s.f. since there are three in 155, 3 in 18.5 and 3 in 0.235. If you round to the nearest even number then 35.65 will be rounded to 35.6. Some may round to 35.7. I suspect either will be counted as correct by your database.
I figured out what I did wrong I divided by 18 and not 18.5. Thank you for your help
To determine how much the temperature will rise when energy is added to a substance, we need to use the formula:
Q = mcΔT
Where:
Q is the energy added (in Joules)
m is the mass of the substance (in grams)
c is the specific heat capacity of the substance (in J/g°C)
ΔT is the change in temperature (in °C)
Given that Q = 155 J, m = 18.5 g, and c = 0.235 J/g°C for silver, we can rearrange the formula:
ΔT = Q / (mc)
Plugging in the values:
ΔT = 155 J / (18.5 g * 0.235 J/g°C)
Calculating the value:
ΔT = 155 J / 4.3275 J/°C
ΔT ≈ 35.8°C
Therefore, the temperature will rise by approximately 35.8°C when 155 J of energy is added to 18.5 g of silver.