Question

multiple choice 1 point
a beaker containing 100 g of water is heated from 20°c to 30°c. how much heat energy (q, in joules, j) was transferred into the water? assume no heat loss to the surroundings.
the specific heat capacity of water is 4.184 j/g°c
q = cp. m. δt
δt = q / cp. m
m = mass of the substance in grams
q = 4.184 joules
q = 41.84 joules
q = 418.4 joules
q = 4184 joules
dont test me yet, i am trying to gain an understanding before attempting to answer this question.

Explanation:

Step1: Identify the formula

The formula for heat transfer is \( q = C_p\cdot m\cdot\Delta T\), where \(C_p\) is the specific - heat capacity, \(m\) is the mass, and \(\Delta T\) is the change in temperature.

Step2: Determine the values of variables

Given \(C_p = 4.184\space J/g^{\circ}C\), \(m=100\space g\), \(\Delta T=T_{final}-T_{initial}=30 - 20=10^{\circ}C\)

Step3: Substitute the values into the formula

Substitute \(C_p = 4.184\space J/g^{\circ}C\), \(m = 100\space g\), and \(\Delta T=10^{\circ}C\) into \(q = C_p\cdot m\cdot\Delta T\)

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Answer:

\(q = 4184\space J\) (the option \(q = 4184\space Joules\))