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3 years ago

A faster pulse rate results in a _____ overall heat input. Answer options are 1. Higher or 2. Lower

Chemistry

2 answers:

kobusy [5.1K]3 years ago

7 0

A faster pulse rate results in a higher overall heat input

shusha [124]3 years ago

3 0

Answer:

higher

Explana

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A 1.26 m aqueous solution of an ionic compound with the formula mx2 has a boiling point of 101.63 ∘c. part a calculate the van't

12345 [234]

Answer is: Van't Hoff factor (i) for this solution is 1.051 .
Change in boiling point from pure solvent to solution: ΔT =i · Kb · b.
Kb - molal boiling point elevation constant is 0.512°C/m.
b - molality, moles of solute per kilogram of solvent.
b = 1.26 m.
ΔT = 101.63°C - 100°C = 1.63°C.

i = 1.63°C ÷ (0.512°C/m · 1.26 m).

i = 1.051.

5 0

3 years ago

Read 2 more answers

This element has 50 electrons in a neutral atom and is usually mixed with metals to form an alloy.

babymother [125]

Heya!

HERE IS YOUR ANSWER:

Electrons = 50

Atomic number = 50

so, the Element is stannum (Sn)

6 0

3 years ago

How many molecules of C 2H 5Br will be present if you had 4.52 g of this compound?

Reptile [31]

Okay ty what what happened to me lol lolhope this helps i lol lol oh yeah that’s okay lol lol yeah lol lol !!! hope it helps :)

5 0

3 years ago

A 0.025-g sample of a compound composed of Boron and hydrogen with the molecular mass of 28 AMU burns spontaneously when exposed

nalin [4]

Answer:

The empirical formula is BH₃ and molecular formula is B₂H₆

Explanation:

To know the number of borons you must obtain the moles number of the initial and B₂O₃ compound. So:

Moles of initial compound:

0,025 g of X × ( 1 mol / 28 g) = 8,9 × 10⁻⁴ moles

Moles of B₂O₃ compound:

AMU of B₂O₃ = (2 × 10,8 g/mol + 3 × 16 g/mol) = 69,6 g/mol

0,063 g ( 1 mol B₂O₃ / 69,6 g) = 9,1 × 10⁻⁴ moles

As moles number of initial and final compounds are the same, the number of borons must be equals. So, our compound has two borons.

These two borons weight: 2 × 10,8 g/mol = 21,6 g/mol

If UMA number of our compound is 28 g/mol we need, yet,

28 g/mol - 21,6 g/mol = 6,4 g/mol

These 6,4 g/mol comes from hydrogen that weights 1 g/mol. So, we have 6 hydrogens.

Thus, the molecular formula is B₂H₆

The empirical formula is the simplest way to represent the atoms of a chemical compound. If we divide the molecular formula in two, we will obtain the empirical formula: BH₃

I hope it helps!

4 0

3 years ago

In CaCo3 + HCl = CaCl2 + H2O +CO3, how many liters of carbon dioxide gas, measured at STP, can be obtained from 45.0 g of calciu

Anon25 [30]

Answer:

B) 10.1 L

Explanation:

Hello,

In this case, for the given chemical reaction which should be corrected as shown below:

$CaCO_3 + HCl \rightarrow CaCl_2 + H_2O +CO_2$

Since 45.0g of calcium carbonate are used, the produced moles of carbon dioxide, via stoichiometry, are found to be:

$n_{CO_2}=45.0g CaCO_3*\frac{1molCaCO_3}{100gCaCO_3}*\frac{1molCO_2}{1molCaCO_3}=0.45molCO_2$

Finally, since STP conditions are referred to a temperature of 273.15K and 1 atm, the volume, by using the ideal gas equation result:

$V=\frac{nRT}{P}=\frac{0.45mol*0.082\frac{atm*L}{mol*K}*273.15K }{1atm} \\ \\V=10.1L$

So the answer is B) 10.1 L.

Best regards.

6 0

3 years ago