A piece of copper with a mass of 22.6 g initially at a temperature of 16.3 °C is heated to a temperature of 33.1 °C. Assuming the specific heat of copper is 0.386 J/(g°C), how much heat was needed for this temperature change to take place?

There is a loss of 0.4 grams. $ 2.0 -1.6$ = 0.4 grams $ 0.4/2.0 xx 100 $ = 20% The Hydrogen will combine with the Oxygen in...

The idea here is that you need to use the mass of copper and the mass of the copper sulfide to determine how much sulfur the produced compound contains, then...

The empirical formulas are $"Cu"_2"O"$ and $"CuO"$. Oxide 1 $color(white)(mmmmml)"Cu" +color(white)(m) "O" → "Oxide 1"$ $"Mass/g":color(white)(l) 2.118color(white)(ll) 0.2666$ Our job is to calculate the ratio of the moles of...

We apply the formula $q=m C Delta T$ mass $m =0.75g$ of copper $C=0.385J g^-1 ºC^-1$ Temperature change $DeltaT=29-7=22ºC$ So, Amount of heat $q=0.75*0.385*22J$ $q=6.3525J$

The heat transferred from the hot metal, is equal to the heat absorbed by the cold water. For the cold water, $ Delta T_w=24-22=2º$ For the metal $DeltaT_o=87-24=63º$ $ m_o...

$q_"gain" = q_"lost"$ $(60g)(92^o - 40^oC)(x) = (70g)(24.5^oC - 40^oC)(4.18)"$ 4.18 is specific of water. Solve for x $3120x=-4535.3$ $x = 4535.3/3120 or 45353/31200$ $x = -1.45362$ This is the...

This is just asking you to know what the units of capacity, $s$, are. After that, this should take you less than a minute: $color(blue)(s_(Ag)) = ("91.5 J/"^@...

The mass of the copper coin is 44.9 g. The formula for the heat absorbed by a substance is $color(blue)(|bar(ul(color(white)(a/a) q = mcΔT color(white)(a/a)|)))" "$...

The formula for the heat absorbed by a substance is $color(blue)(|bar(ul(color(white)(a/a) q = mcΔT color(white)(a/a)|)))" "$ where $q$ is the quantity of heat $m$ is the...

The key here is the of gold, which is said to be equal to $c_"gold" = "0.126 J g"^(-1)""^@"C"^(-1)$ This tells you that in order to increase...