The mass of bismuth carbonate that decomposed is 0.445 g
calculation
write the equation for reaction
that is Bi2(CO3)3 → Bi2O3 +3 CO2
find the moles of of CO2 formed
At STP 1 mole of a gas = 22.4 L
what about 50 Ml
convert the Ml to Liters = 50/1000= 0.05 L
moles of CO2 formed is therefore= 1 mole x 0.05 L/22.4 l =2.232 x10^-3 moles
by use of reacting ratio between Bi(CO3)3 to CO2 which is 1:3 the moles of Bi(CO3)3 is = 2.232 x10^-3 x1/3= 0.744 x10^-4 moles of Bi(CO3)3
mass of Bi(CO3)3 = molar mass x number of moles
mass= 0.744 x10^-4 moles x 597.99 g/mol = 0.445 grams
<u>Answer:</u> The final temperature of the coffee is 43.9°C
<u>Explanation:</u>
To calculate the final temperature, we use the equation:
where,
q = heat released = 
m = mass of water = 10.0 grams
C = specific heat capacity of water = 4.184 J/g°C
= final temperature = ?
= initial temperature = 20°C
Putting values in above equation, we get:
Hence, the final temperature of the coffee is 43.9°C
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