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olasank [31]
2 years ago
14

Calculate the mass of O2 produced after 20.0 grams of KClO3 have reacted?

Chemistry
1 answer:
IrinaVladis [17]2 years ago
5 0

Answer:

RFM \: of \: potassium \: chlorate = (39 + 35.5 + (16 \times 3)) = 122.5 \: g \\ 122.5 \: g \: of \: potassium \: chlorate \: produce \: (16 \times 3) \: g \: of \: oxygen \\ 20.0 \: g \: of \: potassium \: chlorate \: will \: produce \:  (\frac{(20.0 \times 16 \times 3)}{122.5} ) \: g \\  = 7.84 \: g \: of \: oxygen

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Explanation:

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Which of the following statements is true?
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2 years ago
A 80.0 g piece of metal at 88.0°C is placed in 125 g of water at 20.0°C contained in a calorimeter. The metal and water come to
grandymaker [24]

Answer:

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<u>Step 1:</u> Data given

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<u>Step 2:</u> Calculate specific heat of the metal

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with mass of water = 125 grams

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with ΔT(water) = T2-T1 = 24.7 - 20 = 4.7°C

with mass of metal = 80.0 grams

with c(metal) = TO BE DETERMINED

with ΔT(metal) = 24.7 - 88.0 = -63.3 °C

125*4.18*4.7 = -80 * C(metal) * -63.3

2455.75 = -80 * C(metal) * -63.3

C(metal) = 2455.75 / (-80*-63.3)

C(metal) = 0.485 J/g°C

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3 years ago
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Answer:

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E1 reaction always follow Zaitsev’s rule; with E2 reactions, there are exceptions (see antiperiplanar).

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3 years ago
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