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Verizon [17]
3 years ago
11

What are the steps to convert meters to miles

Chemistry
1 answer:
rodikova [14]3 years ago
4 0

m/1,609.344=mi (meters divided by 1,609.344 equals miles)

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algol13
Chechnya. 345. Gcbjshjkfs
3 0
3 years ago
The center on your school’s basketball team is 6 ft 10 in tall. How tall is the player in millimeters (mm)?
svp [43]

The answer is 6 ft 10 inches in millimeters (mm) is 0.833 ft.

Given,

The center of the school's basketball team is 6 ft 10 inches tall.

We have to convert the height of the player from feet and inches to feet.

Using the conversion factor,

1 ft = 12 inches

or, 12inches/ 1 ft

Converting 6ft 10 inches to ft, we get;

10 inches × 1 ft/ 12inches

= 0.833 ft

Therefore 6 ft 10 inches in millimeters (mm) is 0.833 ft.

Unit conversion is a method in which we multiply or divide with a particular numerical factor and then finally round off to the nearest significant digits.

To learn more about Millimeter and Unit conversions, visit: brainly.com/question/26371870

#SPJ4

5 0
1 year ago
Which rule for assigning oxidation numbers is correct?
LenKa [72]
Hydrogen is usually –1. This is INCORRECT. The oxidation number for H is +1.
Oxygen is usually –2. This is CORRECT.
A pure group 1 element is +1. This is INCORRECT. It does not follow. This will depend on the other elements and the overall charge.
A monatomic ion is 0. This is INCORRECT. Diatomic ion is 0.
4 0
3 years ago
Read 2 more answers
If 1.02 g of nickel reacted with 750. mL of 0.112 M hydrobromic acid, how much of each will be present at the end of the reactio
kati45 [8]

Answer:

35.1% is percent yield

Explanation:

<em>Full question: Assume no volume change.  If you formed 0.0910 atm of gas, what is the percent yield?</em>

<em />

The reaction that is occurring is:

Ni + 3HBr → NiBr₃ + 3/2H₂(g)

First, we will determine moles of Ni and HBr to determine limiting reactant and theoretical yield

Using ideal gas law, we can determine the moles of hydrogen formed. Thus, we can find percent yield:

<em>Moles Ni (Molar mass: 58.69g/mol):</em>

1.02g * (1mol / 58.69g) = 0.01738moles Ni

<em>Moles HBr:</em>

0.750L * (0.112mol/L) = 0.084 moles of HBr.

For a complete reaction of the 0.084 moles of HBr you need:

0.084mol HBr * (1 mole Ni / 3 moles HBr) = 0.028 moles of Ni.

As there are just 0.01738 moles of Ni, the Ni is limiting reactant. Assuming a theoretical yield, moles of H₂ produced are:

0.01738moles Ni * (3/2 H₂ / 1 mol Ni) = 0.02607 moles H₂

Now, moles of H₂ produced are:

PV = nRT

PV/RT = n

<em>Where P is pressure (0.0910atm)</em>

<em>V is volume (2.50L)</em>

<em>R is gas constant (0.082atmL/molK)</em>

<em>T is absolute temperature in Kelvin (30°C + 273.15 = 303.15K)</em>

<em>And n are moles</em>

PV/RT = n

0.0910atm*2.50L/0.082atmL/molK*303.15K = n

0.00915 moles = n

<em />

And percent yield (Produced moles / Theoretical moles * 100) is:

0.00915 moles / 0.02607moles =

<h3>35.1% is percent yield</h3>
8 0
2 years ago
If you pump air into cycle tyre a slight warming effect is noticed at valve stem why
Mashutka [201]

As the air molecules move through the valve they have friction as they hit the walls, and its this friction that causes it to heat up.

6 0
3 years ago
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