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polet [3.4K]
3 years ago
5

A researcher wants to experiment with an element that reacts like phosphorus (P) but has a greater atomic mass. Which element sh

ould the researcher select for the experiment?
1.)Nitrogen (N)
2.)Silicon (Si)
3.)Arsenic (As)
4.)Sulfur (S)
Chemistry
2 answers:
IgorC [24]3 years ago
4 0

Answer:

Most likely N or S it might not be safe but that is what experiments do I guess.

Explanation:

wel3 years ago
3 0

Answer:

the answer correct is 4.

sulfur(s)

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Need help ASAP please!
bearhunter [10]

Answer:

13 mol NO

Explanation:

Step 1: Write the balanced equation

4 NH₃(g) + 5 O₂(g) ⇒ 4 NO(g) + 6 H₂O(g)

Step 2: Establish the appropriate molar ratio

According to the balanced equation, the molar ratio of O₂ to NO is 5:4.

Step 3: Calculate the number of moles of O₂ needed to produce 16 moles of NO

We will use the previously established molar ratio.

16 mol O₂ × 4 mol NO/5 mol O₂ = 13 mol NO

3 0
3 years ago
Atmospheric air pressure is measured with a _____.
Svetradugi [14.3K]
It is measured with a barometer
3 0
2 years ago
Read 2 more answers
A tire at 21°C has a pressure of 0.82 atm. Its temperature decreases to –3.5°C. If there is no volume change in the tire, what i
Phantasy [73]
Using ideal gas equation, PV = nRT, and since there is no volume change and amount change, the equation is now P = kT, where k =nR/V. Temperature must be in kelvin From the given, k = (0.82)/ (21 + 273) = 2.78 x 10^-3 Substituting T = -3.5+273, P = 0.75 atm
7 0
3 years ago
Read 2 more answers
A compound containing only carbon, nitrogen, and hydrogen is analyzed to contain 58.82% carbon, 27.45% nitrogen, and 13.73% hydr
Mekhanik [1.2K]
When given percents for an empirical formula problem, first consider all the percents as grams.

58.82% carbon —> 58.82 g carbon
27.45% nitrogen —> 27.45 g nitrogen
13.73% hydrogen —> 13.73 g hydrogen

Then convert the grams of all the elements to moles, based on their molar masses.

Carbon - 58.82 g / 12.01 g/mol = 4.898 mol carbon

Nitrogen - 27.45 g / 14.01 g/mol = 1.959 mol nitrogen

Hydrogen - 13.73 g / 1.008 g/mol = 13.62 mol hydrogen

Then divide all of the mole numbers by the smallest number of moles, which is in this case, the 1.959 mol of nitrogen.

Carbon - 4.898 / 1.959 = 2.5

Nitrogen - 1.959 / 1.959 = 1

Hydrogen - 13.62 / 1.959 = 7

You want whole numbers for all of your mole numbers, so multiply all of them by 2, since 2.5 isn’t a whole number.

Final answer: C5N2H14
4 0
3 years ago
What will result from the Alpha decay of (17 8)O?
Nookie1986 [14]

Answer:

alpha decay, because alpha particles have two protons and two neutrons.  If the isotope has an atomic number two less than the original, it lost two protons, the same amount as in an alpha particle.

Explanation:

3 0
2 years ago
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