current attempt in progress\nhow many joules of heat are required to heat 180 g of aluminum from 16.0 °c to…

current attempt in progress\nhow many joules of heat are required to heat 180 g of aluminum from 16.0 °c to 50.5 °c?\ntable 4.3 | specific heat of selected substances\n| substance | specific heat (j/g°c) | specific heat (cal/g°c) |\n|--|--|--|\n| water | 4.184 | 1.000 |\n| ethyl alcohol | 2.138 | 0.511 |\n| ice | 2.059 | 0.492 |\n| aluminum | 0.900 | 0.215 |\n| iron | 0.473 | 0.113 |\n| copper | 0.385 | 0.0921 |\n| gold | 0.131 | 0.0312 |\n| lead | 0.128 | 0.0305 |\netextbook and media\nsave for later\nattempts: 0

current attempt in progress\nhow many joules of heat are required to heat 180 g of aluminum from 16.0 °c to 50.5 °c?\ntable 4.3 | specific heat of selected substances\n| substance | specific heat (j/g°c) | specific heat (cal/g°c) |\n|--|--|--|\n| water | 4.184 | 1.000 |\n| ethyl alcohol | 2.138 | 0.511 |\n| ice | 2.059 | 0.492 |\n| aluminum | 0.900 | 0.215 |\n| iron | 0.473 | 0.113 |\n| copper | 0.385 | 0.0921 |\n| gold | 0.131 | 0.0312 |\n| lead | 0.128 | 0.0305 |\netextbook and media\nsave for later\nattempts: 0

Answer

Explanation:

Step1: Identify the formula

The formula for heat $Q$ is $Q = mc\Delta T$, where $m$ is the mass, $c$ is the specific - heat capacity, and $\Delta T$ is the change in temperature.

Step2: Determine the values

$m = 180\ g$, $c = 0.900\ J/g^{\circ}C$ (specific heat of aluminum from the table), $\Delta T=T_2 - T_1=50.5^{\circ}C - 16.0^{\circ}C = 34.5^{\circ}C$.

Step3: Calculate the heat

$Q=mc\Delta T=180\ g\times0.900\ J/g^{\circ}C\times34.5^{\circ}C$. $Q = 180\times0.900\times34.5\ J$. $Q = 5589\ J$.

Answer:

$5589$