Use the worked example above to help you solve this problem. An electrical heater is operated by applying a potential difference
of 49.4 V to nichrome wire of total resistance 8.04 Ω. (a) Find the current carried by the wire and the power rating of the heater. I = 6.14 Correct: Your answer is correct. A P = 303.5 Correct: Your answer is correct. W (b) Using this heater, how long would it take to heat 2.10 103 moles of diatomic gas (e.g., a mixture of oxygen and nitrogen, or air) from a chilly 10°C to 25°C? Take the molar specific heat at constant volume of air to be 5 2 R. s (c) How many kilowatt-hours of electricity are used during the time calculated in part (b) and at what cost, at $0.14 per kilowatt-hour? U = kWh cost $ EXERCISEHINTS: GETTING STARTED | I'M STUCK! (a) A hot-water heater is rated at 4.69 103 W and operates at 2.40 102 V. Find the resistance in the heating element and the current. R = Ω I = A (b) How long does it take to heat 125 L of water from 25.6°C to 54.0°C, neglecting conduction and other losses? (The specific heat of water is 4.186 J/g · K.) s (c) How much does it cost at $0.14/kWh? $
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Answer : The mass of silver sulfadiazine produced can be, 71.35 grams.
Solution : Given,
Mass of = 25.0 g
Mass of = 50.0 g
Molar mass of = 231.7 g/mole
Molar mass of = 250.3 g/mole
Molar mass of = 357.1 g/mole
First we have to calculate the moles of and
.
Now we have to calculate the limiting and excess reagent.
The balanced chemical reaction is,
From the balanced reaction we conclude that
As, 2 mole of react with 1 mole of
So, 0.1998 moles of react with
moles of
From this we conclude that, is an excess reagent because the given moles are greater than the required moles and
is a limiting reagent and it limits the formation of product.
Now we have to calculate the moles of
From the reaction, we conclude that
As, 2 mole of react with 2 mole of
So, 0.1998 mole of react with 0.1998 mole of
Now we have to calculate the mass of
Therefore, the mass of silver sulfadiazine produced can be, 71.35 grams.