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MA_775_DIABLO [31]
3 years ago
13

What is the correct name for (NH4)4P407?​

Chemistry
1 answer:
Snowcat [4.5K]3 years ago
3 0

Answer:

Diammonium hydrogen phosphate

Explanation:

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PLEASE HELP!<br> an element with 8 protons and 10 neutrons
leva [86]

Answer:

oxygen ion O2-

Explanation:

because it has 8 protons and gave gained 2 electron so O2-.

6 0
3 years ago
If you were converting from milli- to centi- units, would you move the decimal point to the left or the right
yan [13]

Answer:

Left

Explanation:

6 0
3 years ago
How many significant figures are in the number 0.001022?
Mademuasel [1]

Answer:

4 sig figs.

Explanation:

Significant Figures Rules:

1. Anything that isn't a zero is a sig fig

2. If a decimal point comes after the ones digit, everything before the decimal is counted as sig fig (i.e 2000. would be 4 sig figs).

3. If we are dealing with small decimals, the zero before and after the decimal (i.e 0.002) is a placeholder and is not counted as sig figs.

4. Any zeros between 2 significant digits is considered in sig figs (i.e 2002 would be 4 sig figs).

We look at 0.001022.

We know that 0.00 are not sig figs and are placeholders.

We know that 1022 are significant digits and figures, and we have 4 of them.

Therefore, we have 4 sig figs.

8 0
3 years ago
Read 2 more answers
0.500 L of a gas is collected at 2911 MM and 0°C. What will the volume be at STP?
ioda

Answer:

V₂ =  1.92 L

Explanation:

Given data:

Initial volume = 0.500 L

Initial pressure =2911 mmHg (2911/760 = 3.83 atm)

Initial temperature = 0 °C (0 +273 = 273 K)

Final temperature = 273 K

Final volume = ?

Final pressure = 1 atm

Solution:

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

by putting values,

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 3.83 atm × 0.500 L × 273 K / 273 K × 1 atm

V₂ = 522.795 atm .L. K / 273 K.atm

V₂ =  1.92 L

4 0
3 years ago
HELP ME PLEASEEE
rusak2 [61]

Answer:

68.2%

Explanation:

3 0
3 years ago
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