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Lera25 [3.4K]
3 years ago
9

An electron has a mass of 1) 1 amu 2) -1 amu 3) 0 amu

Chemistry
2 answers:
stira [4]3 years ago
6 0
Electron has a mass of about 9.10938215 × 10 - 31 kg

I will assume 2
Dmitriy789 [7]3 years ago
3 0
Number 2 is the mass of an electron
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S + 6 HNO3 H2SO4 + 6 NO2 + 2 H2O
exis [7]

Answer:

              101.50 g H₂O

Explanation:

The mole ratio of HNO₃ and H₂O is 6 : 2

Hence, 16.9 moles of HNO₃ will produce = 2/6×16.9 = 5.63 moles of H₂O

Also,

Mass = Moles × M.Mass

Mass = 5.63 mol × 18.02 g/mol

Mass = 101.50 g H₂O

5 0
2 years ago
What is number 1 for b, c, and d?
SVETLANKA909090 [29]
B because....................
4 0
3 years ago
Classify each process as either physical or a chemical change.
Dafna11 [192]

Answer:

I think they are all correct

7 0
3 years ago
The arrows represent tge movement of which substances
11111nata11111 [884]
The arrows represent the movement of starting substances
6 0
3 years ago
Nitrogen gas (112 g) reacts with hydrogen gas to produce 40.8 g of ammonia according to the following
Lemur [1.5K]

Answer:

%yield of NH₃ = 30%

Explanation:

Actual yield of NH₃ = 40.8g

Theoretical yield = ?

Equation of reaction

N₂ + 3H₂ → 2NH₃

Molar mass of NH₃ = 17g/mol

Molarmass of N = 14.00

2 molecules of N = 2 * 14.00 = 28g/mol

Number of moles = mass / molar mass

Mass = number of moles * molar mass

Mass = 1 * 28.00 = 28g of N₂ (the number of moles of N₂ from the equation is 1).

From the equation of reaction,

28g of N₂ produce (2 * 17)g of NH₃

28g of N₂ = 34g of NH₃

112g of N₂ = x g of NH₃

X = (112 * 34) / 28

X = 136g of NH₃

Theoretical yield = 136g of NH₃

% yield = (actual yield / theoretical yield) * 100

% yield = (40.8 / 136) * 100

% yield = 0.3 * 100

% yield = 30%

8 0
3 years ago
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