Which statement most accurately describes a chemical equation?

Which metal will more easily lose an electron sodium or potassium?

sergey [27]

<span>The metal that would more easily lose an electron would be potassium. It is more reactive than sodium. Also, looking on the periodic table, </span><span>from top to bottom for groups 1 and 2, reactivity increases. So, it should be potassium. Hope this answers the question. Have a nice day.</span>

7 0

3 years ago

What is the mass percent of nitrogen in ammonium carbonate, (NH4)2CO3?

Margaret [11]

In order for you to calculate for the mass of ammonium carbonate, you need to know the molar mass of it and the nitrogen atoms in the compound. Ammonium carbonate has a molar mass of 96.08 grams per mole. There are two nitrogen atoms in ammonium carbonate which is equal to 28.02 grams per mole. Divide the molar mass of nitrogen to the ammonium carbonate, 28.02/96.08 x 100, we get 29.16wt% nitrogen.

6 0

2 years ago

Why does a higher concentration make a reaction faster?

myrzilka [38]

Option B is correct,
With increase in concentration the density of reactants increases and the system becomes more crowded, the greater the reactants will come in contact with each other and collisions occur. If collision is in proper orientation and has optimum energy then its fruitful and yields product. So, the greater the number of reactants, the greater will be the chances of collision and the greater will be the production of products per unit time and hence, greater is the rate of reaction.

6 0

2 years ago

Read 2 more answers

A sample compound with a molar mass of 34.00g/mol is found to consist of 0.44g H and 6.92g O. Calculate both empirical and molec

balu736 [363]

Answer:

E.F= OH

M.F= $O_{2} H_{2}$

Explanation:

Empirical Formula

Step 1: Calculate mols of each element

0.44gH(1 mol H/ 1.008g H)= 0.4365 mol H

*note leave extra sig figs for calculations

6.92gO(1 mol O/ 16 g O)=0.4325 mol O

Step 2: Identify which is the smallest mol

*in this case 0.4365 mol H> 0.4325 mol O so we will use 0.4325 mol O

Step 3: Divide above calculations by the smallest mol

0.4325 mol O/0.4325= 1

0.4365 mol H/0.4325= 1.009 *rounds to 1

Step 4: use calculations as subscripts

Oxygen = 1 so the subscript will 1 (O)

Hydrogen = 1 so the subscript will 1 (H)

making E.F= OH

Molecular Formula:

Step 1: identify molecular mass and mass from the E.F

the molecular mass is given 34.00g/mol

the mass of the E.F is

(oxygen mass from periodic table)+(hydrogen mass from periodic table)

16+1.008= 17.008

Step 2:Divide the molecular mass by the mass given by the emipirical formula.

$\frac{34.00}{17.008}= 1.999$ round to 2

Step 3:Multiply the empirical formula (the subscripts) by this number to get the molecular formula. ANSWER: M.F=2(OH)- $O_{2} H_{2}$

3 0

2 years ago

A geologist working in a national park finds a mineral. He is carrying a kit that contains a penny, a hand lens, a piece of tile

Verizon [17]

A penny for the scratch test (low hardness)a hand lens for inspection a peice of tile for a streak test a geologic hammer to test for cleavage of fracture and the pocket knife for the scratch test (high hardness)

6 0

3 years ago