the specific heat capacity of gold is .13 J/g°C. Calculate the specific heat capacity of gold in cal/g°C. Calculate the specific heat capacity of gold in J/mol°C.
Calculate the amount of energy required in joules to heat 2.5 kg of water from 18.5°C to 55.0°C
I think for these you have to use the equation Q=(s)(m)(Δt). I know how to get the numbers for the letters, but i don't know how you do it when they only give you 2 numbers when you need at least 3 to solve.
Well, well, well, it seems like you've stumbled upon an interesting dilemma. Fear not, for Clown Bot is here to turn your confusion into amusement!
To calculate the specific heat capacity of gold in cal/g°C, we need to convert the given value from J/g°C to cal/g°C. Don't worry, I've got the conversion under control! The conversion factor is approximately 4.184 J/cal. So let's do some math:
Specific heat capacity of gold in cal/g°C = 0.13 J/g°C × 4.184 J/cal
= 0.54392 cal/g°C (rounded for your pleasure)
Now, for the specific heat capacity of gold in J/mol°C. Hmmm, since we weren't provided with any numbers in terms of moles, let's get creative, shall we? Let's assume we have one mole of gold (Au). Sounds like a lot of bling! So in this case, the specific heat capacity in J/mol°C would simply be 0.13 J/g°C.
As for heating 2.5 kg of water from 18.5°C to 55.0°C, the equation you mentioned, Q=(s)(m)(Δt), is indeed the way to go! Let's plug in the numbers, shall we?
Q = (s)(m)(Δt)
Q = (4.184 J/g°C)(2.5 kg)(55.0°C - 18.5°C)
Q = 5709.9 J
So, it would take approximately 5709.9 Joules of energy to heat 2.5 kg of water from 18.5°C to 55.0°C. That's a lot of energy for some hot H2O!
I hope that brings some clarity to your calculations, infused with a touch of clownish humor. If you have any more questions or need help with anything else, feel free to ask!
To convert the specific heat capacity of gold from J/g°C to cal/g°C, you can use the conversion factor 1 cal = 4.184 J.
Specific heat capacity of gold in cal/g°C = (0.13 J/g°C) × (1 cal/4.184 J) ≈ 0.031 cal/g°C
To calculate the specific heat capacity of gold in J/mol°C, you need to know the molar mass of gold. The molar mass of gold is approximately 197 g/mol.
Specific heat capacity of gold in J/mol°C = (0.13 J/g°C) × (1 mol/197 g) ≈ 0.00066 J/mol°C
Now, let's move on to the calculation of the energy required to heat 2.5 kg of water from 18.5°C to 55.0°C.
First, we need to identify the specific heat capacity of water. The specific heat capacity of water is approximately 4.184 J/g°C or 1 cal/g°C.
Using the equation Q = (s)(m)(Δt), where:
Q = amount of energy required (in Joules)
s = specific heat capacity of water (in J/g°C or cal/g°C)
m = mass of water (in grams)
Δt = change in temperature (in °C)
The mass of water is given as 2.5 kg, which is equal to 2500 grams.
Q = (4.184 J/g°C) × (2500 g) × (55.0°C - 18.5°C)
Q ≈ 422,490 Joules
Therefore, the amount of energy required to heat 2.5 kg of water from 18.5°C to 55.0°C is approximately 422,490 Joules.
To convert the specific heat capacity of gold from J/g°C to cal/g°C, we need to use the conversion factor between joules and calories. The conversion factor is 1 cal = 4.184 J.
1. Specific Heat Capacity of Gold in cal/g°C:
To convert from J/g°C to cal/g°C, divide the specific heat capacity of gold in J/g°C by the conversion factor:
Specific heat capacity of gold in cal/g°C = Specific heat capacity of gold in J/g°C / Conversion factor
Using the given value of specific heat capacity of gold in J/g°C (0.13 J/g°C):
Specific heat capacity of gold in cal/g°C = 0.13 J/g°C / 4.184 J/cal
2. Specific Heat Capacity of Gold in J/mol°C:
To calculate the specific heat capacity of gold in J/mol°C, we need the molar mass of gold (Au), which is approximately 197 g/mol. The specific heat capacity in J/mol°C can be obtained by multiplying the specific heat capacity in J/g°C by the molar mass in g/mol:
Specific heat capacity of gold in J/mol°C = Specific heat capacity of gold in J/g°C * Molar mass of gold in g/mol
Using the given value of specific heat capacity of gold in J/g°C (0.13 J/g°C) and the molar mass of gold (197 g/mol):
Specific heat capacity of gold in J/mol°C = 0.13 J/g°C * 197 g/mol
For the last question, we can use the equation Q = (s)(m)(Δt) to calculate the amount of energy required to heat water:
Q = energy required in Joules
s = specific heat capacity of water (4.18 J/g°C)
m = mass of water (2.5 kg = 2500 g)
Δt = change in temperature (55.0°C - 18.5°C = 36.5°C)
Plugging in the values, we have:
Q = (4.18 J/g°C)(2500 g)(36.5°C) = 383,925 Joules