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denpristay [2]
3 years ago
11

In HNO3, the oxidation state of hydrogen is +1 and the oxidation state of oxygen is -2. Therefore, the oxidation state of nitrog

en is -
Chemistry
1 answer:
marta [7]3 years ago
4 0
+1 Because of all the numbers of charges -2+1+x=0 so, the number should be 1 for the oxidation of H.
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Use the ideal gas law to calculate the pressure in atmospheres of 0.21 mol of helium (He) at 16°C & occupying 2.53 L. You mu
chubhunter [2.5K]

Answer:

The answer to your question is 2.32 atm

Explanation:

Data

P = ?

n = 0.214

V = 2.53 L

T = 61°C

R = 0.082 atm L/mol°K

Formula

PV = nTR

solve for P

P = nRT/V

Process

1.- Calculate the temperature in K

°K = °C + 273

°K = 61 + 273

    = 334

2.- Substitution

P = (0.214 x 0.082 x 334) / 2.53

3.- Simplification

P = 5.86/2.53

4.- Result

P = 2.32 atm

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3 years ago
A 30.0g sample of O2 at standard temperature and pressure (STP) would occupy what volume in liters
Murrr4er [49]

Answer:

Explanation:

A 30.0g sample of O2 at standard temperature and pressure (STP) would occupy what volume in liters

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30 gm of O2 is 30/32= 0.94 =n

PV = nRT

at STP: P= 1 atm, T=273 K, R is always 0.082 for P in atm and T in K

SO

1 X V = 0.94 X 0.082 X 273

using high school freshman algebra,

V= 0.94 X 0.082 X 273 = 21L

using high school algebra I,

V=

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2 years ago
In n=6 the correct sequence for filling of electron will be​
Novay_Z [31]

Answer:

there are 2 ways

2,4

or

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3 years ago
How do human beings prepare their food<br>​
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Well they buy food then they cook it then they eat it
3 0
3 years ago
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Someone explain it plz​
timofeeve [1]

Answer:

1). 1 mole of Carbon burnt in air

C + O2 →CO2

1 mole of carbon produces 1 mole of CO2 which is 44g of CO2

2). 1 mole of carbon is burnt in 16g of dioxygen

32g of O2 = 44g of CO2

1g of O2 = 44/32

CO2 (Dioxygen is limiting reagent)

16g of O2 = 4/32 × 16 = 22g of CO2 in one mole

3) 2 moles of Carbon burnt in 16g of dioxygen

16g of dioxygen is available, and thus it can combine with 0.5 mol of carbon to give 22g of CO2

4 0
2 years ago
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