# How do you calculate final temperature with specific heat?

Subtract the final and initial temperature to get the change in temperature (ΔT). Multiply the change in temperature with the mass of the sample. Divide the heat supplied/energy with the product. The formula is C = Q / (ΔT ⨉ m) .

## What is the formula of final temperature?

For our purposes, we will rearrange the specific heat equation to yield the increase in temperature (ΔT=Qm⋅c Δ T = Q m ⋅ c ), then use that with a rearranged equation for the change in temperature to find the final temperature (Tf=Ti+ΔT T f = T i + Δ T ).

## What is the formula to calculate temperature?

1. Celsius to Kelvin: K = C + 273.15.
2. Kelvin to Celcius: C = K – 273.15.
3. Fahrenheit to Celcius: C = (F-32) (5/9)
4. Celsius to Fahrenheit: F = C(9/5) + 32.
5. Fahrenheit to Kelvin: K = (F-32) (5/9) + 273.15.
6. Kelvin to Fahrenheit: F = (K-273.15) (9/5) + 32.

## What is Q MC ∆ T used for?

The amount of heat gained or lost by a sample (q) can be calculated using the equation q = mcΔT, where m is the mass of the sample, c is the specific heat, and ΔT is the temperature change.

## What is Q in Q MC ∆ T?

Q = mc∆T. Q = heat energy (Joules, J) m = mass of a substance (kg) c = specific heat (units J/kg∙K)

## What is the final temperature of the mixture of 50g of steam?

Answer: The final temperature will be 0°C.

## What would be the final temperature of a mixture of 50g of 20?

Let the specific heat capacity of water be S. Hence, the final temperature of a mixture of 50g of water at 20°C temperature and 50g of water at 40°C temperature would be 30°C.

## How do you find the initial temperature in chemistry?

Q = mc(T – t0) So this rewritten form of the equation makes it simple to find initial temperature. You can plug in all the other values that you’re given, then solve for t0. For example: Say you add 75.0 Joules of energy to 2.0 grams of water, raising its temperature to 87 °C.

## What are the 3 formulas of heat?

• H = (VI)t.
• H = (I 2 R)t.
• H = (V 2 /R)t.

## How do you calculate Q in thermodynamics?

Thus, in the equation ΔU=q+w w=0 and ΔU=q. The internal energy is equal to the heat of the system. The surrounding heat increases, so the heat of the system decreases because heat is not created nor destroyed. Therefore, heat is taken away from the system making it exothermic and negative.

## What does Q stand for in thermodynamics?

Q is the net heat transferred into the system—that is, Q is the sum of all heat transfer into and out of the system. W is the net work done on the system.

## What is the final temperature of the calorimeter?

The final temperature of the calorimeter is 59.0 °C. Now that we know the heat capacity of our calorimeter we can use our calorimeter to determine the amount of heat a reaction releases.

## What is the final temperature when 20.0 g of water at 20 C is mixed with 30.0 g of water at 80 C the specific heat of water is 4.18 JG Co?

The final temperature of the water will be 31.2 °C.

## What will be the final temperature if 50 gram of water at zero degree Celsius is added to 250 gram of water at 90 degree Celsius?

Heat lost by 250g of water at 90°c will be equal to heat gained by 50g of water at exactly 0°c. If heat lose/gain from the environment are neglected, Heat lost by 250g of water at 90°c will be equal to heat gained by 50g of water at exactly 0°c.

## What is the temperature of mixture if 10g of steam at 100 C is mixed with 50g of ice at 0 C?

Hence, the final temperature of the mixture is 100C.

## What would be the final temperature of 50 grams?

Answer: since it is given that 50 gms water at 20 ⁰ C and 50 gms of water at 40⁰ C are mixed. Since the masses of the liquid at different temperatures are same, the answer is very easy and simple : average of 20⁰C and 40⁰C. that is: 30⁰C.