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3 years ago

Which of the following properly lists the metals in order from decreasing to increasing ease of oxidation?

2 answers:

6 0

I know it is either B or D, since I know that K will oxidize in water, and Ag will have a tougher time oxidizing. I am going to lean towards D for my answer.

lora16 [44]3 years ago

6 0

Answer is: D. Ag < Cu < Cr < K.

Reactivity series is an empirical progression of a series of metals, arranged by their reactivity from highest to lowest (alkaline metals have highest reactivity and Noble metals lowest reactivity):

K > Ba > Sr > Na > Ca > Mg > Be > Al > Mn > Zn > Cr> Fe > Cd > Co > Ni > Sn > Pb > H(in acids) > Cu > Hg > Ag.

Metal higher in the reactivity series will displace another and it will be oxidized.

For example, potassium is more reactive than silver.

Chemical reaction: K + AgCl → KCl + Ag.

Potassium is oxidized (from oxidation number 0 to +1) and silver is reduced (from oxidation number +1 to 0).

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How many moles of oxygen are needed to burn 2.7 moles of methyl

QveST [7]

Answer:

3.38 moles of O2.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

4CH2OH + 5O2 → 4CO2 + 6H2O

From the balanced equation above,

4 moles of CH2OH required 5 moles of O2 for complete combustion.

Finally, we shall determine the number of mole of O2 needed to react with 2.7 moles of CH2OH. This can be obtained as follow:

From the balanced equation above,

4 moles of CH2OH required 5 moles of O2 for complete combustion.

Therefore, 2.7 moles of CH2OH will require = (2.7 × 5)/4 = 3.38 moles of O2 for complete combustion.

Thus, 3.38 moles of O2 is required.

5 0

3 years ago

I want to balance S+O2 = SO3

Gre4nikov [31]

Answer:

2S +3O2 =2SO3

Explanation:

2 at the front of sulphur is to equalize the 2 put in SO3.

7 0

3 years ago

Read 2 more answers

From a laboratory process, a student collects 28.0 g of hydrogen and 224.0 g of oxygen. how much water was originally involved i

nikklg [1K]

Chemical reaction is given as :

$2H_{2}O\rightarrow 2H_{2}+O_{2}$

Here, 2 moles of water gives 2 moles of hydrogen and one mole of oxygen.

Mass of hydrogen = 28.0 g (given)

Mass of oxygen = 224.0 g (given)

Number of moles = $\frac{given mass}{molar mass}$

Thus, number of moles of hydrogen = $\frac{28 g}{2\times 1 g/mol}$

= 14 moles of hydrogen

Number of moles of oxygen= $\frac{224 g}{2\times 16 g/mol}$

= 7 moles of oxygen

Now, to find the amount of water:

$7 mol of oxygen \times (\frac{2 mol of water}{1 mol of oxygen})\times (18 g/mol of water)$

= 252 g of water.

Thus, amount of water is 252 g (involved in the process).

4 0

4 years ago

Calculate the molality of a solution containing 257 g glucose (c6h12o6) dissolved in 1.62 l of water. assume a density of 1.00 g

Alex777 [14]

Molality is defined as the number of moles of solute in 1 kg of solvent.
since density and volume has been given we can calculate the mass of water
mass = density x volume
mass = 1.00 g/mL x 1620 mL = 1620 g
number of moles of glucose - 257 g / 180 g/mol = 1.43 mol
number of moles of glucose in 1620 g - 1.43 mol
therefore number of moles in 1000 g - 1.43 mol / 1.620 kg = 0.883 mol/kg
therefore molality is 0.883 mol/kg

4 0

4 years ago

Which condition must be met in order for an equation to be balanced? The elements in the reactants are the same as the elements

Nookie1986 [14]

Answer:

There must be an equal amount of each element on both sides of the equation.

Hope this helps

good luck

8 0

3 years ago

Read 2 more answers