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Given the Following: heat of fusion of ice = 80.0 cal/g; specific heat of ice = 0.480 cal/g; and specific heat of water = 1.00 cal/g. Calculate the amount of heat required to melt 30.0 g of ice at 0 degrees celsius?

Md Ariful Islam

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Md Ariful Islam

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$H_2O(s) +DeltararrH_2O(l)$.......

Note that BOTH the ice and water have a specified temperature of $0$ $""^@C$, and thus we assess the heat involved in the phase change, and thus we only need the $"latent heat of fusion of ice"$, $80.0*cal*g^-1$.

And for the given quantity, this $80*cal*g^-1xx30*g=2400*cal$; whatever a $"calorie"$ is...........

By the same token, we would report the enthalpy change of the reverse reaction......

$H_2O(l) +DeltararrH_2O(s)$, $DeltaH^@=-2400*cal$. Do you agree?

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A250. mL sample of gas at 1.00 atm and 20 degrees Celsius has the temperature increased to 40 degrees Celsius and the volume increased to 500. mL. What is the new pressure?

$(P_1V_1)/T_1=(P_2V_2)/T_2$, given a constant quantity of gas. And thus, $(P_1xxV_1xxT_2)/(V_2xxT_1)=P_2$, even given this format, we can see the problem is dimensionally sound. We do need to use $"absolute temperature."$ $P_2=(1.00*atmxx250*mLxx313*K)/(500*mLxx293*K)~=1/2*atm.$

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Concept of is to be applied here. Let the partial pressure of $Ar$ in the final mixture be $p_"Ar"$ Initially before mixing $ Ar$ had Pressure $P_"Ar"=1.29$ atm Temperature$T_"Ar"=223+273=500$...

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Here's how I go about doing this. What we can do is use the ideal gas equation for both $"Ar"$ and $"O"_2$ to find the total moles. Then we...

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The Arrhenius equation looks like this $color(blue)(|bar(ul(color(white)(a/a)k = A * "exp"(-E_a/(RT))color(white)(a/a)|)))" "$, where $k$ - the rate constant for a given reaction $A$ - the pre-exponential factor, specific...

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What amount of energy is required to melt a 10.7 g piece of ice at 0 C? The heat of fusion of ice = 333 Jg-1

We perform the physical reaction........ $H_2O(s) +Deltararr H_2O(l)$; both reactants and products are at $0$ $""^@C$, and thus we need only assess the energy transfer of the PHASE change........ We...

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How much heat is required to convert 20.0 g of ice at -50.0°C to liquid water at 0.0°C? The specific heat of ice is 2.06 J/(g *$"^o$C) and the heat of fusion of water is 334 J/g?

We interrogate the process..... $H_2O(s)stackrel(Delta_1, -20^@C...0^@C)rarrH_2O(s)stackrel(Delta_2=Delta_"fusion")rarrH_2O(l)$ Now $Delta_1=20.0*gxx2.06*J*g^-1*""^@C^-1xxDeltaT=$ $20.0*gxx2.06*J*g^-1*""^@C^-1xx50$ $""^@C=2060*J$ And $Delta_2=20.0*gxx334*J*g^-1=$ $20.0*gxx334*J*g^-1=6680*J$ $"Total heat"=Delta_1+Delta_2=2060*J+6680*J=??*J$

1 Answers 1 views
The heat of fusion for water is 80. cal/g. How many calories of heat are needed to melt a 35 g ice cube that has a temperature of 0 C?

The formula for the heat required to melt a solid is $color(blue)(|bar(ul(color(white)(a/a) q= mΔ_"fus"H^°color(white)(a/a)|)))" "$ where $q = "the amount of heat"$ $m = "the mass...

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What amount of heat is required to melt $"300 g"$ of ice at its freezing point if the enthalpy of fusion is $"6.02 kJ/mol"$?

For a phase transition, we assume a constant temperature (and also, pressure). So, the heat flow $q$ into a substance is equal to the change $DeltaH$. $bb(q_P)$ $= bb(mDeltaH)$,...

1 Answers 1 views
The latent heat of fusion for ice is 6.0 kJ/mole. In order to melt 36 g of ice (solid $H_2O$) at 0°C, how much energy is required?

The molar latent heat of fusion, which is an alternative name given to the of fusion, tells you how much heat is required in order to convert a specific...

1 Answers 1 views

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