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3 years ago

NEED ANSWER ASAP ! WILL BRAINLIST !

Chemistry

1 answer:

nydimaria [60]3 years ago

6 0

It’s C hope it helps :) : new processes
Will be developed to locate the trees more efficiently

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A disturbance in matter that carries energy from one place to another is called

siniylev [52]

The answer you're looking for is: a wave.

6 0

3 years ago

Given that nitrogen forms three bonds with hydrogen to make <img src="https://tex.z-dn.net/?f=NH_%7B3%7D" id="TexFormula1" title

lbvjy [14]

Answer:

Three hydrogen atoms to form PH₃.

Explanation:

Hello!

In this case, since the elements belonging to the nitrogen family (N, P, As, Sb and Bi) show five valence electrons, because there are five electrons at their outer shell, it is clear that if phosphorous bonds with hydrogen, it is going to require the same amount of oxygen atoms (3) because elements having five valence electrons need 3 bonds in order to attain the octet (5+3=8).

Therefore the compound would be:

$PH_3$

Which is phosphine.

Best regards!

3 0

3 years ago

A certain liquid has a vapor pressure of 92.0 Torr at 23.0 °C and 351.0 Torr at 45.0 °C. Calculate the value of ΔH°vap for this

notka56 [123]

There is a specific formula to use for these type of problems.

ln (P2/ P1)= Δvap/ R x (1/T1 - 1/T2)

R= 8.314
P1= 92.0 torr
T1= 23 C + 273= 296 K
P2= 351.0 torr
T2= 45.0 C + 273= 318 K

plug the values and solve for the unknown

ln( 351.0/ 92.0)= Δvap/ 8.314 x (1/296 - 1/318)

Δvap= 47630.6 joules

3 0

3 years ago

Read 2 more answers

The molar volume of a gas at STP, in liters, is

pashok25 [27]

Answer: 22.4L

Gas at STP means gas at standard temperature and pressure of one mole of an ideal gas

Ideal gas Law PV=nRT

Standard pressure is 1atm or 22.4L

Standard temperature is 273.15K

Any questions feel free to ask. Thanks

3 0

3 years ago

Nicotine, a component of tobacco, is composed of c, h, and n. a 4.200-mg sample of nicotine was combusted, producing 11.394 mg o

Rudiy27

Answer:

Empirical Formula = C₅H₇N₁

Solution:

Data Given:

Mass of Nicotine = 4.20 mg = 0.0042 g

Mass of CO₂ = 11.394 mg = 0.011394 g

Mass of H₂O = 3.266 mg = 0.003266 g

Step 1: Calculate %age of Elements as;

%C = (mass of CO₂ ÷ Mass of sample) × (12 ÷ 44) × 100

%C = (0.011394 ÷ 0.0042) × (12 ÷ 44) × 100

%C = (2.7128) × (12 ÷ 44) × 100

%C = 2.7128 × 0.2727 × 100

%C = 73.979 %

%H = (mass of H₂O ÷ Mass of sample) × (2.02 ÷ 18.02) × 100

%H = (0.003266 ÷ 0.0042) × (2.02 ÷ 18.02) × 100

%H = (0.7776) × (2.02 ÷ 18.02) × 100

%H = 0.7776 × 0.1120 × 100

%H = 8.709 %

%N = 100% - (%C + %H)

%N = 100% - (73.979 % + 8.709%)

%N = 100% - 82.688%

%N = 17.312 %

Step 2: Calculate Moles of each Element;

Moles of C = %C ÷ At.Mass of C

Moles of C = 73.979 ÷ 12.01

Moles of C = 6.1597 mol

Moles of H = %H ÷ At.Mass of H

Moles of H = 8.709 ÷ 1.01

Moles of H = 8.6227 mol

Moles of N = %N ÷ At.Mass of O

Moles of N = 17.312 ÷ 14.01

Moles of N = 1.2356 mol

Step 3: Find out mole ratio and simplify it;

C H N

6.1597 8.6227 1.2356

6.1597/1.2356 8.6227/1.2356 1.2356/1.2356

4.985 6.978 1

≈ 5 ≈ 7 1

Result:

Empirical Formula = C₅H₇N₁

6 0

3 years ago